Question

In: Chemistry

If you mix equal concentrations of reactants and products, which of the following reaction proceed to...

If you mix equal concentrations of reactants and products, which of the following reaction proceed to the right and which proceed to the left?

a. H2CO3(aq) + HSO4− (aq) ⇌ H2SO4(aq) + HCO3− (aq)

b. HF(aq) + Cl− (aq) ⇌ HCl(aq) + F− (aq)

c. HF(aq) + NH3(aq) ⇌ NH4 + (aq) + F− (aq)

d. HSO4− (aq) + CN− (aq) ⇌ HCN(aq) + SO42−(aq)

e. [Al(H2O)6] 3+(aq) + OH− (aq) ⇌ [Al(H2O)6(OH)]2+ (aq) + H2O(l)

Solutions

Expert Solution

The question can be answered on the basis of the relative strengths of acids and bases. It must be noted that a strong acid reacts to form a weak acid. The same thing holds true for bases: a strong base proceeds to form a weak base.

a) H2CO3 (aq) + HSO4- (aq) <=====> HCO3- (aq) + H2SO4 (aq)

H2SO4 is a much stronger acid than H2CO3; hence, the reverse reaction is favored, i.e, the reverse reaction proceeds to form more H2CO3.

b) HF (aq) + Cl- (aq) <======> F- (aq) + HCl (aq)

HCl is a much stronger acid than HF; hence, the reverse reaction is favored and more HF is produced.

c) HF (aq) + NH3 (aq) <=====> F- (aq) + NH4+ (aq)

HF is a stronger acid than NH4+; hence, the reaction proceeds in the forward direction to produce more NH4+.

d) HSO4- (aq) + CN- (aq) <=====> SO42- (aq) + HCN (aq)

HSO4- is a much stronger acid than HCN; hence, the reaction proceeds to the right to give HCN.

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

Calculating Equilibrium Concentrations The concentrations of reactants and products for a chemical reaction can be calculated...
Calculating Equilibrium Concentrations The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. Part A Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g),    Kc=7.20 If only COF2 is present initially at a concentration of 2.00 M, what concentration of...
The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium...
The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g),    Kc=7.40 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Consider...
The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium...
The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. Consider the reaction CO(g)+NH3(g)⇌HCONH2(g),    Kc=0.890 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium? Please show all steps! Thank you!
For the reaction shown below, the initial concentrations for reactants and products are as follows: [A]...
For the reaction shown below, the initial concentrations for reactants and products are as follows: [A] = 0.27 M, [B] = 0.0640 M, [C] = 0.0134 M, and [D] = 1.47 M. If the equilibrium constant for the reaction is KC = 0.802, which direction does the reaction have to shift to reach equilibrium? A + 3B ⇌ 2C + 3D Enter 1 if it shifts left, 2 if it shifts right, or 3 if it's already at equilibrium.
The equilibrium concentrations of the reactants and products were measured for the following chemical reaction. PCl3(g)...
The equilibrium concentrations of the reactants and products were measured for the following chemical reaction. PCl3(g) + Cl2(g) equilibrium reaction arrow PCl5(g) equilibrium concentrations: [PCl3] = 0.203 M [Cl2] = 0.203 M [PCl5] = 0.939 M At a certain temperature, the equilibrium constant, Kc, for this reaction, is 94.1. If an additional 0.250 M PCl3 is added to the system, determine the new equilibrium concentrations of PCl3, Cl2, and PCl5.
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) Kc = 17; [NH3] = 0.50 M, [N2] = 0.15 M, [H2] = 0.12 M (b) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) KP = 6.8 × 104 ; initial pressures: NH3 = 2.00 atm, N2...
The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium.
  The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA+bB⇌cC+dD the Kc and Kp expressions are given by Kc=[C]c[D]d/[A]a[B]b Kp=(PC)c(PD)d(PA)a(PB)b The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their...
For a reaction in which the products contain more energy than the reactants, which of the...
For a reaction in which the products contain more energy than the reactants, which of the following is true? A. There is a negative change in free energy B. Delta G < 0 C. The reaction requires energy input D. The reaction occurs spontaneously E. The reaction is called exergonic Part 2: Which of the following best describes the process of aerobic respiration? A. The electrons from glucose are donated to ADP transforming it into ATP, which the cells uses...
For the following reaction, the products are favored at equilibrium. Classify each of the reactants and...
For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. HC9H7O4 + (C2H5)2NH<--->(C2H5)2NH2+ + C9H7O4-
A reaction was run with two different initial concentrations of reactants A and B: Experiment A...
A reaction was run with two different initial concentrations of reactants A and B: Experiment A / M B / M rateB / (M/sec) 1 0.00022 0.00046 0.0841 2 0.00022 0.00166 0.3035 What is the order of the reaction with respect to B? A reaction was run with two different initial concentrations of reactants A and B: Experiment A / M B / M rateB / (M/sec) 1 0.00057 0.00067 0.0000825 2 0.00057 0.00621 0.0657 What is the order of...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT